Name: _______________________________________
Chapter 13 Vocabulary – Honors
Date: ______________________
1) allotrope –
A different form of the same substance in the same state of matter. I.E. diamond and
graphite – both made of carbon but clearly are very different.
2) amorphous solid –
Glass, plastic, rubber – solids that are non-crystalline – the particles that make it up
do not have order.
3) atmospheric pressure –
The pressure exerted by the atmosphere on a given system. Decreases at higher
altitudes.
4) barometer –
A tool for measuring atmospheric pressure. Atmospheric pressure can be measured
in mm Hg, torr, atmospheres, or kPa (kilopascals)
5) boiling point The temperature at which a given liquid substance transitions to the gas phase. At
this temperature, vapor pressure equals atmospheric pressure.
6) crystal A solid that is rigid and has a crystalline shape – particles that compose it are in
order or show a repeating pattern. Essentially the opposite of an amorphous solid.
7) evaporation The process of a given liquid transitioning to the gas phase. Essentially the same as
vaporization, except evaporation happens for a liquid that is NOT boiling.
8) gas pressure –
Pressure exerted by a gas on its container.
9) glass An example of an amorphous solid.
10) kinetic energy The energy of motion. All molecules at temperatures above 0 K have kinetic energy
and are in motion.
Name: _______________________________________
Chapter 13 Vocabulary – Honors
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11) kinetic theory A theory that all particles in each state of matter have motion at all times and
temperatures above 0 K.
12) melting point The temperature at which a given solid substance transitions to the liquid phase.
Same as freezing point.
13) normal boiling point Boiling point of a liquid at normal atmospheric pressure (101.3 kPa). At higher
altitudes, atmospheric pressure decreases and so does boiling point.
14) pascal A unit of measurement for pressure. 1000 pascals equals 1 kilopascal. Symbol is Pa;
kilopascal is kPa.
15) phase diagram A diagram illustrated the states of matter of a given substance at different
temperatures and pressures.
16) plasma A state of matter of substances at high temperatures. Made of hot ions.
17) standard atmosphere Normal atmospheric pressure. This is equal to 760mm Hg, 760 torr, 101.3 kPa, or 1
atm.
18) sublimation The process of a solid transitioning directly to the gas phase without first becoming
a liquid. The opposite is called deposition.
19) triple point The temperature and pressure point on a phase diagram in which regions that
designate solid, liquid, and gas all come together. Under these conditions, all three
states of matter for the same substance can exist at the same time. Usually located
toward the “lower left” of the diagram (at relatively low temperature and pressure).
Name: _______________________________________
Chapter 13 Vocabulary – Honors
Date: ______________________
20) unit cell The smallest group of particles of a solid crystal that has the shape of the crystal.
Similar to the idea that the smallest particle of an element that retains the element’s
chemical characteristics is the atom (below that, the element is NOT unique, just like
going smaller than a unit cell makes a crystal NOT unique).
21) vacuum –
A space in which there are no gas particles. Essentially a region with no matter.
Outer space is a vacuum.
22) vapor pressure –
The pressure of a gas against the process of evaporation. The stronger the vapor
pressure in a closed container, the less evaporation can take place. Vapor pressure
is responsible for why boiling point decreases at higher altitudes (less vapor
pressure).
23) vaporization –
The process of a given liquid transitioning to the gas phase. Essentially the same as
evaporation, except vaporization happens as a liquid is boiling.